Answer: the pressure exerted by the gas is 652 x 10^3 Pa, which corresponds to 652 kPa
Explanation:
The question requires us to calculate the pressure, in kPa, connsidering the following information:
<em>number of moles = n = 4.20mol</em>
<em>volume of gas = V = 15.0L</em>
<em>temperature of gas = T = 280.0 K</em>
We can use the equation of ideal gases to calculate the pressure of the gas, as shown by the rearranged equation below:
Since the volume was given in L and the question requires us to calculate the pressure in kPa, we can use R in units of L.Pa/K.mol:
<em>R = 8314.46 L.Pa/K.mol</em>
Applying the values given by the question to the rearranged equation above, we'll have:
Therefore, the pressure exerted by the gas is 652 x 10^3 Pa, which corresponds to 652 kPa.
Answer:
the answer is 18 atoms [your welcome]
<u>Answer:</u> The partial pressure of carbon dioxide having solubility 0.886g/100mL is 4182.4 mmHg
<u>Explanation:</u>
Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.
The equation given by Henry's law is:
......(1)
where,
= solubility of carbon dioxide in water = 0.161 g/100 mL
= Henry's constant = ?
= partial pressure of carbon dioxide = 760 mmHg
Putting values in equation 1, we get:
Now, calculating the pressure of carbon dioxide using equation 1, we get:
= solubility of carbon dioxide in water = 0.886 g/100 mL
= Henry's constant = 4720.5 g.mmHg/100 mL
= partial pressure of carbon dioxide = ?
Putting values in equation 1, we get:
Hence, the partial pressure of carbon dioxide having solubility 0.886g/100mL is 4182.4 mmHg
Answer:
Explanation:
First write all numerators above the common denominator
4/5 - 1/2 - 1/2=
- 1/2
Subtract the numbers
- 1/2 =
-
Write all numerators above the least common denominator 10
- =
Subtract the numbers and you got your answer :)
Answer:
Transition Element
Explanation:
Transition elements are defined as those elements which can form at least one stable ion and has partially filled d-orbitals. They are also characterized by forming complex compounds and having different oxidation states for a single metal element.
Transition metals are present between the metals and the non metals in the periodic table occupying groups from 3 to 12. There general electronic configuration is as follow,
(n-1)d
¹⁻¹⁰ns
¹⁻²
The general configuration shows that for a given metal, the d sublevel will be in lower energy level as compared to corresponding s sublevel. For example,
Scandium is present in fourth period hence, its s sublevel is present in 4rth energy level so its d sublevel will be present in 3rd energy level respectively.
Hence, we can conclude that for transition metals the electron are present in highest occupied s sublevel and a nearby d sublevel
.